If the concentration of`[NH_(4)^(+)]` in a solution having 0.02 M `NH_(3)`and 0.005 M Ca `( OH)_(2)` is `a xx 10^(-6) ` M,determine a.
`[k_(b) ( NH_(3)) = 1.8 xx 10^(-5) ]`

What is [NH_(4)^(+)] in a solution that contain 0.02 M NH_(3)(K_(b)=1.8xx10^(-5)) and 0.01 M KOH?

What is [NH_(4)^(+)] in a solution that contain 0.02 M NH_(3)(K_(b)=1.8xx10^(-5)) and 0.01 M KOH?

What is [NH_(4)^(+)] in a solution that contain 0.02 M NH_(3)(K_(b)=1.8xx10^(-5)) and 0.01 M KOH?

What [NH_4^(+) ] in a solution that contains 0.02M NH_3 (K_b =1.8 xx 10^(-5) ) and 0.01 M KOH ?

A solution consist of 0.2 M NH_(4)OH and 0.2 M NH_(4)Cl . If K_(b) of NH_(4)OH is 1.8 xx 10^(-5) , the [OH^(-)] of the resulting is

What is pH of 0.02 M solution of ammonium chloride at 25^(@) C ? K_(b) (NH_(3)) = 1.8 xx 10^(-5) .

What is pH of 0.02 M solution of ammonium chloride at 25^(@) C ? K_(b) (NH_(3)) = 1.8 xx 10^(-5) .

Calculate the molar solubility of Fe(OH)_(3) in a buffer solution that is 0.1M in NH_(4)OH and 0.1M in NH_(4)Cl (K_(b) of NH_(4)OH=1.8xx10^(-5) , K_(sp) of Fe(OH)_(3)=2.6xx10^(-39) )